A sample of gas originally at 29.2°C and 1.847 atm pressure in a 5.53 L container is allowed to expand until the pressure is 0.357 atm and the temperature is 23.6°C. The final volume of the gas is Record your answer with 3 significant figures.

A cylinder is filled with  10.0L  of gas and a piston is put into it. The initial pressure of the gas is measured to be  147.kPa . The piston is now pulled up, expanding the gas, until the gas has a final volume of  72.0L . Calculate the final pressure of the gas. Round your answer to  3  significant digits.

A 6.00 L tank at 14.5 °C is filled with 10.2 g of sulfur tetrafluoride gas and 5.04 g of carbon dioxide gas. You can assume both gases behave as ideal gases under these conditions. Calculate the partial pressure of each gas in the tank. Be sure your answers have the correct number of significant digits. sulfur tetrafluoride carbon dioxide partial pressure: partial pressure: 0 atm atm 10 X

A 9.00 L tank at 19.4 °C is filled with 2.75 g of chlorine pentafluoride gas and 13.9 g of sulfur hexafluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the partial pressure of each gas in the tank. Be sure your answers have the correct number of significant digits. chlorine pentafiuoride partial pressure: sulfur hexafluoride partial pressure: ? atm

A 9.00 L tank at 3.79 °C is filled with 8.94 g of sulfur tetrafluoride gas and 13.3 g of sulfur hexafluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to 3 significant digits. sulfur tetrafluoride sulfur hexafluoride mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: 0 0 0 atm atm atm X

A 10.0 L tank at 14.2 °C is filled with 19.3 g of sulfur hexafluoride gas and 3.57 g of dinitrogen monoxide gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to 3 significant digits. sulfur hexafluoride dinitrogen monoxide mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: 8 atm atm atm D X

A 10.0 L tank at 14.2 °C is filled with 6.58 g of dinitrogen difluoride gas and 14.7 g of sulfur tetrafluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Be sure your answers have the correct number of significant digits. dinitrogen difluoride sulfur tetrafluoride mole fraction: partial pressure: mole fraction: partial pressure: Total pressure in tank: 0 0 atm 0 0 atm atm x10 X Ś

Some N₂ gas is mixed with some O₂ gas, and the sketch below shows a representative sample of the mixture. The total pressure of the mixture is measured, and found to be 0.150 kPa. gas N₂ 0₂ carbon nitrogen kPa oxygen mole fraction partial pressure kPa key Calculate the mole fraction and partial pressure of each gas in this mixture. Round your answers to 3 significant digits. You may assume each gas behaves as an ideal gas. hydrogen x10 sulfur chlorine × Ś

A 6.00 L tank at 7.53 °C is filled with 5.91 g of sulfur hexafluoride gas and 7.97 g of boron trifluoride gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction and partial pressure of each gas, and the total pressure in the tank. Round each of your answers to 3 significant digits. mole fraction: sulfur hexafluoride partial pressure: ? atm mole fraction: boron trifluoride partial pressure: atm Total pressure in tank: atm